Find the pH of each mixture of acids. Acid Ionization Constants (Ka) for Some Monoprotic Weak Acids at 25 ∘C Acid Formula Ka Benzoic acid HC7H5O2 6.5×10−5 Hydrofluoric acid HF 6.8×10−4 Phenol HC6H5O 1.3×10−10 Formic acid HCHO2 1.8×10−4 Hypochlorous acid HClO 2.9×10−8

Find the pH of each mixture of acids. Acid Ionization Constants (Ka) for Some Monoprotic Weak Acids at 25 ∘C Acid Formula Ka Benzoic acid HC7H5O2 6.5×10−5 Hydrofluoric acid HF 6.8×10−4 Phenol HC6H5O 1.3×10−10 Formic acid HCHO2 1.8×10−4 Hypochlorous acid HClO 2.9×10−8

A.) 0.070 M in HNO3 and 0.185 M in HC7H5O2 Express your answer to two decimal places.

B.) 0.025 M in HBr and 0.020 M in HClO4 '

C.) 0.095 M in HF and 0.230 M in HC6H5O

a) the pH of the mixture = 1.13

b) the pH of this mixture  = 1.35

c) the pH of this mixture  = 2.09

Explanation:

The formula to determine the hydrogen ion concentration in benzoic acid is as follows:

HNO₃ is a strong acid whose dissociation is complete and thorough into its ions.

So, = 0.070 M

The total hydrogen concentration of the mixture will now be:

= (0.0035 + 0.070 )M

= 0.0735 M

Now the pH can be determined as:

pH = - log

pH = - log [0.0735]

pH = - (-1.13)

pH = 1.13

Hence, the pH of the mixture = 1.13

b) In HBr and HClO₄, these are both strong acids and as such, they undergo complete dissociation of their ions.

So,

So,

The total hydrogen ion concentration of the mixture =

Now; the pH will be

pH = - log

pH = - log [0.045]

pH = - (-1.35)

pH = 1.35

Thus, the pH of this mixture  = 1.35

c) For hydrofluoric acid and phenol (weak acids ), the following expression is used to calculate the hydrogen ion concentration

The pH can then be calculated as follows:

pH = - log

pH = - log  [0.008037]

pH = - (-2.09)

pH = 2.09

Thus, the pH of this mixture  = 2.09